Educational institutes, especially colleges and universities, focus on science and emerging subjects to help students thrive in each aspect of life. Chemistry is also a part of advanced sciences, and theoretical yield is an important part of this subject to estimate the real amount of the expected product.
If you don’t know how to find theoretical yield, read the following information, as I have discussed the whole process comprehensively. So, why wait?
Allow Me To Proceed!
What is Theoretical Yield?
Theoretical yield is the maximum calculated amount of product from a balanced chemical equation. However, environmental conditions are considered ideal while analyzing the process to prevent any loss.
In finding theoretical yield, all limiting reactants (due to which reaction stops or completes) are converted into the product (perfect transformation).
The theoretical yield is always greater than the actual yield because of normal environmental conditions. Also, these conditions aren’t ideal for a theoretical chemical process.
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- Actual Yield is the real amount of reactant that converts into a product with all losses during the reaction. It is always less than the theoretical yield due to different losses.
- Percentage Yield is the ratio of actual yield to theoretical yield, which is multiplied by a hundred.
Percentage Yield = Actual Yield x 100/Theoretical Yield
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How to Find Theoretical Yield?
In the section below, I have gathered some easy steps to guide you on how to find theoretical yield. Here, I have taken the following reactant:
- Hydrogen
- Oxygen
I have taken one molecule of each element to proceed with the process because neither element exists in singular forms.
H2 + O2 → H2O
Number of Atoms
H=2, O=2 → H=2, O=1
The above equation is the chemical equation of water formation. However, this equation is not balanced. That means that the number of atoms of each element on the right side of the equation is not equal to the number of atoms on the left side.
Now, balance the equation by multiplying the specific element, molecule, or compound to match the number of atoms on both sides.
2H2 + O2 → 2H2O
Number of Atoms
H=4, O=2 → H=4, O=2
The above equation is balanced by multiplying Hydrogen with “2” and water with “2.” Hydrogen has 4 atoms, and Oxygen has 2 atoms on both sides.
This is a chemical reaction of the process of “Water” formation.
4H2 +2O2 → 4H2O
Using the periodic table, find out the molar mass of each element. After that, multiply the molar mass of each reactant by its number of atoms.
At the end, add all the molar mass of all reactants. According to the periodic table, the molar mass of Hydrogen and Oxygen is as follows:
H=1 , O=16
H : O
H=4, O=2
4(1) : 2(16)
Molar Mass
4 : 32
In an experiment, the amount of reactants is known. Suppose you have 5 grams of Hydrogen and 10 grams of Oxygen.
To convert the amount of reactant from grams to moles, divide the available amount by the molar mass of each reactant.
H2 : O
4/5 : 32/10
From Grams to Moles
0.8 : 3.2
For this purpose, divide the amount of Hydrogen by the amount of Oxygen.
H2 : O
0.8 : 3.2
0.25
Now, divide the coefficient of Hydrogen by the coefficient of Oxygen.
H2 : O
No. of Molecules
4 : 2
Dividing
4/2
Result
2
Compare the ratios of both elements and determine which element remains and which is completely utilized in the reaction.
H2 : O
Ratios of elements
0.25 : 2
Comparing
0.25 < 2
From the above equation, it is obvious that Hydrogen is the limiting reactant and Oxygen is the excess reactant, as some of its amount remains unreacted after the reaction.
That showcases Hydrogen as a limiting reactant.
To find theoretical yield, first, divide the number of molecules of the product by the number of molecules of the limiting reactant.
H2O : H2
No. of Molecules
4 : 4
Dividing
4/4
Result
1
Now, multiply the result by the amount of your limiting reactant in moles. Then, you will get the ‘Theoretical Yield.’
Amount of limiting reactant (H2) in moles = 0.8
Theoretical yield = 0.8 ✕ 1
Theoretical yield= 0.8
Now, multiply the theoretical yield by the molar mass of the product to convert it into grams and get your answer. Here is the process of how to find theoretical yield in grams.
Theoretical yield = 0.8
The molar mass of the product ( H2O) = 18
To convert Theoretical yield in grams = 0.8 ✕ 18
= 14.4g
The Closing Note
Well, in the above section, I have compiled the whole process in step by step guide on how to find theoretical yield in Chemistry for education. Theoretical yield is calculated under ideal conditions without any by-products or losses.
Due to these reasons, the theoretical yield is not achievable, and the actual yield is the yield obtained in reality with all losses. So, if you have any questions, then let me know in the comments.
Please let me know what you think of it!
